(B) The precipitation of $BaCO_3$ begins when the ionic product exceeds the solubility product constant $(K_{sp})$.$K_{sp} = [Ba^{2+}][CO_3^{2-}]$Give

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

(B) The precipitation of $BaCO_3$ begins when the ionic product exceeds the solubility product constant $(K_{sp})$.$K_{sp} = [Ba^{2+}][CO_3^{2-}]$Given $K_{sp} = 5.1 \times 10^{-9}$ and $[CO_3^{2-}] = 1.0 \times 10^{-4} \, M$.Substituting the values:$5.1 \times 10^{-9} = [Ba^{2+}] \times 1.0 \times 10^{-4}$$[Ba^{2+}] = \frac{5.1 \times 10^{-9}}{1.0 \times 10^{-4}}$$[Ba^{2+}] = 5.1 \times 10^{-5} \, M$

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Solubility product

Medium

Solid $Ba(NO_3)_2$ is gradually dissolved in $1.0 \times 10^{-4} \, M \, Na_2CO_3$ solution. At which concentration of $Ba^{2+}$ will the precipitation begin? $(K_{sp} \, BaCO_3 = 5.1 \times 10^{-9})$

A
$4.1 \times 10^{-5} \, M$
B
$5.1 \times 10^{-5} \, M$
C
$8.1 \times 10^{-8} \, M$
D
$8.1 \times 10^{-7} \, M$

Explore More

Browse All

Question Bank

All Subjects

Class 11 Questions

Class 11

Chemistry Questions

Chapter

6-2.Equilibrium-II (Ionic Equilibrium)

Subtopic

Solubility product

When equal volumes of the following solutions are mixed,precipitation of $AgCl$ $(K_{sp} = 1.8 \times 10^{-10})$ will occur only with:

MediumIIT 1988

View Solution

If the $K_{sp}$ of $Mg(OH)_2$ is $1 \times 10^{-12}$,at what $pH$ will $Mg(OH)_2$ precipitate from a $0.01 \ M$ solution of $Mg^{2+}$ ions?

Medium

View Solution

When equal volumes of $Ca^{2+}$ and $F^{-}$ solutions are mixed,in which of the solutions precipitation will not occur? $(K_{sp} \text{ of } CaF_2 = 1.6 \times 10^{-10})$

MediumAP EAMCET 2020

View Solution

Why only $As^{3+}$ gets precipitated as $As_2S_3$ and not $Zn^{2+}$ as $ZnS$ when $H_2S$ is passed through an acidic solution containing $As^{3+}$ and $Zn^{2+}$?

MediumAIIMS 2013

View Solution

Which of the following happens when $NH_{4}OH$ is added gradually to the solution containing $1 \ M \ A^{2+}$ and $1 \ M \ B^{3+}$ ions?
Given: $K_{sp}[A(OH)_{2}] = 9 \times 10^{-10}$ and $K_{sp}[B(OH)_{3}] = 27 \times 10^{-18}$ at $298 \ K$.

DifficultJEE MAIN 2025

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

Solid $Ba(NO_3)_2$ is gradually dissolved in $1.0 \times 10^{-4} \, M \, Na_2CO_3$ solution. At which concentration of $Ba^{2+}$ will the precipitation begin? $(K_{sp} \, BaCO_3 = 5.1 \times 10^{-9})$

Similar Questions

When equal volumes of the following solutions are mixed,precipitation of $AgCl$ $(K_{sp} = 1.8 \times 10^{-10})$ will occur only with:

If the $K_{sp}$ of $Mg(OH)_2$ is $1 \times 10^{-12}$,at what $pH$ will $Mg(OH)_2$ precipitate from a $0.01 \ M$ solution of $Mg^{2+}$ ions?

When equal volumes of $Ca^{2+}$ and $F^{-}$ solutions are mixed,in which of the solutions precipitation will not occur? $(K_{sp} \text{ of } CaF_2 = 1.6 \times 10^{-10})$

Why only $As^{3+}$ gets precipitated as $As_2S_3$ and not $Zn^{2+}$ as $ZnS$ when $H_2S$ is passed through an acidic solution containing $As^{3+}$ and $Zn^{2+}$?

Which of the following happens when $NH_{4}OH$ is added gradually to the solution containing $1 \ M \ A^{2+}$ and $1 \ M \ B^{3+}$ ions? Given: $K_{sp}[A(OH)_{2}] = 9 \times 10^{-10}$ and $K_{sp}[B(OH)_{3}] = 27 \times 10^{-18}$ at $298 \ K$.

Vedclass Test Series

Exam Paper Generator

Online Exam Module

Which of the following happens when $NH_{4}OH$ is added gradually to the solution containing $1 \ M \ A^{2+}$ and $1 \ M \ B^{3+}$ ions?
Given: $K_{sp}[A(OH)_{2}] = 9 \times 10^{-10}$ and $K_{sp}[B(OH)_{3}] = 27 \times 10^{-18}$ at $298 \ K$.